Question

Titanium tetrachloride, TiCₗ4, has a melting point of −23.2 °C and has a ΔH fusion = 9.37 kJ/mol.

a. How much energy is required to melt 263.1 g TiCl₄?
b. For TiCl₄, which will likely have the larger magnitude: ΔH fusion or ΔH vaporization?

a) q = 5.07 kJ, ΔH vaporization is larger.
b) q = 2.47 kJ, ΔH fusion is larger.
c) q = 9.37 kJ, ΔH vaporization is larger.
d) q = 2.47 kJ, ΔH vaporization is larger.

Answer 1

The energy required to melt 263.1 g of TiCl4 is 13.00 kJ, and the enthalpy of vaporization for TiCl4 would likely have a larger magnitude than the enthalpy of fusion.

Step-by-step explanation:

Answer to Titanium Tetrachloride Melting

To calculate the energy required to melt 263.1 g of titanium tetrachloride (TiCl4), we first need to convert grams to moles using the molar mass of TiCl4, which is 189.68 g/mol. The calculation is as follows:

263.1 g ÷ 189.68 g/mol = 1.387 mol

Now, using the given enthalpy of fusion (ΔH fusion = 9.37 kJ/mol), the total energy needed is:

1.387 mol × 9.37 kJ/mol = 13.00 kJ

As for the second part of the question, enthalpy of vaporization is generally larger than the enthalpy of fusion because the former involves breaking more intermolecular forces as a substance transitions from liquid to gas, compared to the fusion which involves a solid to liquid transition.

So, both provided answer options are incorrect.